2) Using curved arrows, show how each of the two species below can act as a Lewis base and a Lewis acid. a) Water and hydrogen chloride. b) Acetic acid and a strong base, dimethylamide. c) Aluminum chloride and trimethylamine.
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In this case, hydrogen chloride can act as a Lewis acid by accepting the lone pair of electrons from water. H2O + HCl -> H3O+ + Cl- Water can also act as a Lewis acid by accepting a lone pair of electrons from a Lewis base. In this case, hydrogen chloride can Show more…
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Using curved arrows, show how the species in part (a) can act as Lewis bases in their reactions with HCl, and show how the species in part (b) can act as Lewis acids in their reaction with $\mathrm{OH}^{-}$ (a) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}, \mathrm{HN}\left(\mathrm{CH}_{3}\right)_{2}, \mathrm{P}\left(\mathrm{CH}_{3}\right)_{3}$ (b) $\mathrm{H}_{3} \mathrm{C}^{+}, \mathrm{B}\left(\mathrm{CH}_{3}\right)_{3}, \mathrm{MgBr}_{2}$
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Identify each of the following species as either a Lewis acid or a Lewis base, and write an equation illustrating a Lewis acid-base reaction for each one. Use curved arrows to depict electron-pair movement. Be sure that the product of each reaction is depicted by a complete, correct Lewis structure. (a) $\mathrm{CN}^{-}$ (b) $\mathrm{CH}_{3} \mathrm{OH}$ (c) $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CH}^{+}$ (d) $\mathrm{MgBr}_{2}$ (e) $\mathrm{CH}_{3} \mathrm{BH}_{2}$ (f) $\mathrm{CH}_{3} \mathrm{~S}^{-}$
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